Oxygen difluoride



Oxygen difluoride
Other names difluorine monoxide
fluorine monoxide
oxygen difluoride
oxygen fluoride
hypofluorous anhydride
Identifiers
CAS number [7783-41-7]
Properties
Molecular formula OF2
Molar mass 53.9962 g mol−1
Melting point

−224 °C

Boiling point

−145 °C

Solubility in other solvents 68 mL gaseous OF2 in 1 L (0 °C)[1]
Thermochemistry
Std enthalpy of
formation ΔfHo298 		24.5 kJ mol−1
Related Compounds
Related compounds SCl2
Except where noted otherwise, data are given for
materials in their standard state
(at 25 °C, 100 kPa)
Infobox disclaimer and references

Oxygen difluoride is the oxidant.

Preparation

Oxygen difluoride was first reported in 1929; it was obtained by the electrolysis of molten potassium fluoride and sodium hydroxide:

2F2 + 2NaOH → OF2 + 2NaF + H2O

Reactions

Its powerful oxidizing properties are suggested by the radical mechanism.

OF2 reacts with many metals to yield XeF4 and xenon oxyfluorides.

Oxygen difluoride reacts very slowly with water to form hydrofluoric acid:

OF2(aq) + H2O(aq) → 2HF(aq) + O2(g)

Popular culture

In Robert L. Forward's science fiction novel Camelot 30K, oxygen difluoride was used as a biochemical solvent by fictional life forms living in the solar system's Kuiper belt.

Safety

OF2 is a dangerous chemical, as is the case for any strongly oxidizing gas.

References

  1. ^ Yost, D. M. "Oxygen Fluoride" Inorganic Syntheses, 1939 volume, 1, pages 109-111.
  2. ^ Lebeau, P.; Damiens, A. "A New Method for the Preparation of the Fluorine Oxide”Compt. rend. 1929, volume 188, 1253-5.
  3. ^ Lebeau, P.; Damiens, A. "The Existence of an Oxygen Compound of Fluorine"Compt. rend. 1927, volume 185, pages 652-4.
 
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